J. Chem. Eng. Data 2000, 45, 559-563
559
Densities and Viscosities of Binary Mixtures of Toluene with Methanol, Ethanol, Propan-1-ol, Butan-1-ol, Pentan-1-ol, and 2-Methylpropan-2-ol at (303.15, 308.15, 313.15) K Pandharinath S. Nikam,* Bapu S. Jagdale, Arun B. Sawant, and Mehdi Hasan P. G. Department of Physical Chemistry, M.S.G. College, Malegaon Camp-423105, India
Densities and viscosities of the binary mixtures of toluene with methanol, ethanol, propan-1-ol, butan1-ol, pentan-1-ol, and 2-methylpropan-2-ol have been measured at 303.15, 308.15, and 313.15 K. From these data, excess molar volumes (VE) and deviations in viscosity (∆η) have been calculated. These results are fitted to Redlich-Kister type polynomial equations to estimate the binary coefficients and standard errors.
Introduction Thermodynamic and transport properties of binary liquid mixtures containing protic, aprotic, and associated liquids have been studied in earlier literature.1-5 The calculated excess quantities from such data have been interpreted in terms of the differences in the size of molecules and the strength of specific and nonspecific interactions taking place between components of the mixtures. In this study, the interaction of alkanols with toluene has been investigated. Alkanols exist in associated form whereas toluene has a nonassociated structure in the liquid state. When alkanols are mixed with toluene, mixing properties with varying intermolecular interactions may be generated. To investigate this effect, in the present investigation, the density (F) and the viscosity (η) of binary mixtures of methanol, ethanol, propan-1-ol, butan-1-ol, pentan-1-ol, or 2-methylpropan-2-ol with toluene have been studied over the entire range of composition at (303.15, 308.15, and 313.15) K. Before this study, very few reports6 were available in the literature on the density of the mixtures, but no reports on the viscosity were available. Experimental Section Toluene (Qualigens Fine Chemicals, purity > 99%) was double distilled, and the middle fraction was used.7 Ethanol (Maharashtra Government Distillary) was refluxed over calcium oxide for 5 h and distilled at atmospheric pressure. This procedure was repeated two or three times.8 Methanol (Quilignens Fine Chem, purity 99%), propan-1-ol (E. Merck, purity 99.5%), butan-1-ol (s. d. fine chem., purity 99%), and 2-methylpropan-2-ol (s. d. fine chem., purity 99.2%) were used after single distillation. The purity of the solvents after purification was ascertained by GLC and also by comparing their densities and viscosities with the corresponding literature values at 303.15 K (Table 1). Binary mixtures were prepared by mass in airtight, stoppered glass bottles with a precision of (0.01 mg on a Metler balance (Switzerland, model AE-240). Care was taken to avoid evaporation and solvent contamination during mixing. The estimated error in mole fraction was 200 s and the capillary radius (0.5 mm) was far less than its length (50-60 mm), the kinetic energy and the end corrections were negligible. The dynamic viscosity (η) of the liquids was calculated using
η/η0 ) (Ft)/(F0t0)
(1)
where F, F0 and t, t0 refer to the density and the flow time of the liquids and water, respectively. The values of the dynamic viscosities (η) thus obtained are reproducible to (0.003 mPa‚s. The other experimental details of the measurements of density and viscosity remain the same as those described previously.12 Results and Discussion Experimental values of densities (F) and viscosities (η) of mixtures at (303.15, 308.15, and 313.15) K are listed as a function of mole fraction of toluene in Table 2. The F values have been used to calculate the excess molar volumes (VE) using the following equation:
VE/(cm3mol-1) ) (x1M1 + x2M2)/F12 (x1M1/F1) - (x2M2/F2) (2) where F12 is the density of the mixture and x1, M1, F1 and x2, M2, F2 are the mole fraction, the molecular weight, and the density of pure components 1 and 2, respectively. The viscosity deviations (∆η) were calculated using
∆η/(mPa‚s) ) η12 - x1η1 - x2η2
10.1021/je990317i CCC: $19.00 © 2000 American Chemical Society Published on Web 05/13/2000
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Journal of Chemical and Engineering Data, Vol. 45, No. 4, 2000
Table 1. Comparison of Experimental Densities (G) and Viscosities (η) of Pure Liquids with Literature Values along with Deviations (δ) at 303.15 K F/(g‚cm-3)
η/(mPa‚s)
liquid
expt
lit.
δ (%)
expt
lit.
δ (%)
toluene methanol ethanol propan-1-ol butan-1-ol pentan-1-ol 2-methylpropan-2-ol
0.8566 0.7816 0.7806 0.7954 0.8024 0.8068 0.7750
0.8569(2) 0.7816(16), 0.7817(8) 0.7806(8), 0.7805(16) 0.7956(8), 0.7955(12) 0.8022(8), 0.8020(12) 0.8072(8), 0.8068(18) 0.7755(8), 0.7755(12)
0.03 0.00 0.01 0.01 0.25 0.00 0.06
0.526 0.514 0.965 1.705 2.246 2.973 3.359
0.527(7) 0.5146(8), 0.515(12) 0.976(19) 1.705(16), 1.725(8) 2.262(15) 2.909(8), 2.961(18) 3.378(8), 3.318(17)
0.19 0.12 1.45 0.00 0.71 0.40 0.56
Table 2. Density (G), Viscosity (η), and Excess Molar Volume (VE) for Toluene (1) + Alkanols (2) at (303.15, 308.15, and 313.15) K x1
F (×10-3)
VE
(kg‚m-3)
(cm3‚mol-1)
0.0000 0.0912 0.2105 0.2773
0.7816 0.7978 0.8136 0.8204
0.0000 0.0912 0.2105 0.2773
0.7769 0.7930 0.8087 0.8155
0.0000 0.0692 0.1849 0.3191
0.7806 0.7900 0.8036 0.8136
0.0000 0.0692 0.1849 0.3191
0.7762 0.7855 0.7989 0.8117
0.0000 0.1141 0.1926 0.2912
0.7954 0.8052 0.8114 0.8184
0.0000 0.1141 0.1926 0.2912
0.7913 0.8010 0.8071 0.8140
0.0000 0.1141 0.1926 0.2912
0.7871 0.7967 0.8027 0.8095
0.0000 0.0859 0.2006 0.2972
0.8024 0.8078 0.8144 0.8198
0.0000 0.0859 0.2006 0.2972
0.7985 0.8038 0.8102 0.8155
0.0000 0.0859 0.2006 0.2972
0.7945 0.7996 0.8059 0.8112
η
F (×10-3)
VE
(mP‚s)
(kg‚m-3)
(cm3‚mol-1)
x1
-0.034 -0.073 -0.085
0.514 0.531 0.539 0.542
0.3723 0.4963 0.6944 0.8307
-0.031 -0.065 -0.077
0.480 0.495 0.502 0.504
0.3723 0.4963 0.6944 0.8307
-0.031 -0.062 -0.068
0.965 0.893 0.803 0.699
0.5285 0.5858 0.6901 0.7906
-0.025 -0.053 -0.062
0.881 0.814 0.736 0.642
0.5285 0.5858 0.6901 0.7906
η
F (×10-3)
VE
η
(mPa‚s)
x1
(kg‚m-3)
(cm3‚mol-1)
(mPa‚s)
0.540 0.529 0.515 0.513
0.8880 0.9511 1.0000
0.8535 0.8553 0.8566
-0.033 -0.016
0.516 0.520 0.526
0.502 0.494 0.482 0.481
0.8880 0.9511 1.0000
0.8486 0.8505 0.8518
-0.027 -0.011
0.483 0.488 0.496
0.596 0.575 0.546 0.527
0.8565 0.9213 1.0000
0.8500 0.8531 0.8566
0.030 0.019
0.519 0.524 0.526
0.552 0.533 0.507 0.491
0.8565 0.9213 1.0000
0.8452 0.8483 0.8518
0.037 0.023
0.486 0.493 0.496
0.8737 0.9517 1.0000
0.8506 0.8543 0.8566
0.048 0.023
0.541 0.527 0.526
Toluene (1) + Methanol (2) 303.15 K 0.8285 -0.096 0.8368 -0.097 0.8466 -0.078 0.8516 -0.047 0.8236 0.8319 0.8418 0.8468
308.15 K -0.090 -0.088 -0.071 -0.043
Toluene (1) + Ethanol (2) 303.15 K 0.8320 -0.035 0.8353 0.003 0.8414 0.027 0.8467 0.033 0.8272 0.8306 0.8366 0.8419
308.15 K -0.027 0.014 0.034 0.040
Toluene (1) + Propan-1-ol (2) 303.15 K 0.8240 -0.017 0.866 0.8299 0.012 0.761 0.8380 0.045 0.651 0.8441 0.056 0.587
-0.034 -0.045 -0.039
1.705 1.376 1.182 0.982
0.3778 0.4778 0.6242 0.7421
-0.032 -0.042 -0.036
1.526 1.251 1.078 0.899
0.3778 0.4778 0.6242 0.7421
0.8195 0.8254 0.8334 0.8394
308.15 K -0.012 0.016 0.050 0.062
0.795 0.703 0.608 0.553
0.8737 0.9517 1.0000
0.8458 0.8495 0.8518
0.053 0.028
0.514 0.499 0.496
-0.030 -0.038 -0.030
1.372 1.150 0.990 0.830
0.3778 0.4778 0.6242 0.7421
0.8150 0.8208 0.8288 0.8347
313.15 K -0.005 0.024 0.057 0.067
0.736 0.655 0.570 0.521
0.8737 0.9517 1.0000
0.8411 0.8447 0.8470
0.057 0.033
0.491 0.476 0.471
0.999 0.833 0.726 0.590
0.8121 0.9470 1.0000
0.8470 0.8540 0.8566
0.073 0.023
0.571 0.526 0.526
Toluene (1) + Butan-1-ol (2) 303.15 K 0.8248 0.073 0.8310 0.090 0.8362 0.094 0.8445 0.084
-0.004 0.034 0.056
2.246 1.860 1.452 1.175
0.3877 0.5025 0.6013 0.7617
-0.001 0.041 0.068
1.982 1.656 1.311 1.065
0.3877 0.5025 0.6013 0.7617
0.8204 0.8264 0.8316 0.8398
308.15 K 0.084 0.109 0.109 0.095
0.911 0.770 0.675 0.557
0.8121 0.9470 1.0000
0.8423 0.8492 0.8518
0.080 0.027
0.534 0.498 0.496
0.003 0.053 0.080
1.764 1.489 1.193 0.979
0.3877 0.5025 0.6013 0.7617
0.8159 0.8219 0.8269 0.8351
313.15 K 0.106 0.129 0.130 0.109
0.840 0.713 0.629 0.524
0.8121 0.9470 1.0000
0.8376 0.8444 0.8470
0.097 0.035
0.507 0.478 0.471
Journal of Chemical and Engineering Data, Vol. 45, No. 4, 2000 561 Table 2 (Continued) x1
F (×10-3)
VE
(kg‚m-3)
(cm3‚mol-1)
η
F (×10-3)
VE
(mP‚s)
(kg‚m-3)
(cm3‚mol-1)
0.0000 0.0745 0.2114 0.4291
0.8068 0.8103 0.8167 0.8272
0.026 0.065 0.099
2.973 2.508 1.810 1.101
0.0000 0.0745 0.2114 0.4291
0.8030 0.8064 0.8126 0.8229
0.031 0.077 0.114
2.592 2.202 1.611 1.001
0.0000 0.0745 0.2114 0.4291
0.7992 0.8025 0.8086 0.8186
0.036 0.088 0.128
2.262 1.940 1.439 0.911
0.0000 0.1003 0.1723 0.3109
0.7750 0.7820 0.7872 0.7984
0.257 0.415 0.505
3.359 1.981 1.455 0.986
0.0000 0.1003 0.1723 0.3109
0.7698 0.7768 0.7820 0.7933
0.268 0.420 0.513
2.623 1.622 1.239 0.878
0.0000 0.1003 0.1723 0.3109
0.7645 0.7716 0.7767 0.7882
0.264 0.431 0.520
2.014 1.328 1.059 0.781
x1
η
F (×10-3)
VE
η
(mPa‚s)
x1
(kg‚m-3)
(cm3‚mol-1)
(mPa‚s)
0.8629 0.9443 1.0000
0.8492 0.8536 0.8566
0.058 0.032
0.564 0.536 0.526
0.8629 0.9443 1.0000
0.8445 0.8488 0.8518
0.073 0.039
0.530 0.507 0.496
0.8629 0.9443 1.0000
0.8397 0.8440 0.8470
0.093 0.047
0.500 0.484 0.471
0.8135 0.9107 1.0000
0.8405 0.8484 0.8566
0.290 0.213
0.549 0.521 0.526
0.8135 0.9107 1.0000
0.8355 0.8435 0.8518
0.305 0.223
0.518 0.490 0.496
0.8135 0.9107 1.0000
0.8305 0.8386 0.8470
0.322 0.234
0.486 0.460 0.471
Toluene (1) + Pentan-1-ol (2) 303.15 K 0.5202 0.8317 0.106 0.925 0.6090 0.8361 0.113 0.787 0.7058 0.8410 0.101 0.678 0.8063 0.8462 0.079 0.592 308.15 K 0.5202 0.8273 0.122 0.846 0.6090 0.8316 0.132 0.726 0.7058 0.8364 0.118 0.630 0.8063 0.8416 0.093 0.554 313.15 K 0.5202 0.8229 0.140 0.778 0.6090 0.8271 0.150 0.670 0.7058 0.8318 0.140 0.587 0.8063 0.8368 0.116 0.520 Toluene (1) + 2-Methylpropan-2-ol (2) 303.15 K 0.3886 0.8047 0.541 0.854 0.4942 0.8135 0.535 0.727 0.6059 0.8228 0.496 0.644 0.7118 0.8317 0.419 0.588 308.15 K 0.3886 0.7996 0.550 0.771 0.4942 0.8084 0.541 0.666 0.6059 0.8178 0.500 0.594 0.7118 0.8266 0.436 0.547 313.15 K 0.3886 0.7945 0.554 0.696 0.4942 0.8034 0.549 0.611 0.6059 0.8127 0.515 0.548 0.7118 0.8216 0.454 0.510
Table 3. Parameters and Standard Deviations (σ) of Eqs 3 and 4 for Toluene + Alkanols system toluene + methanol
VE/(cm3‚mol-1) ∆η/(mPa‚s)
toluene + ethanol
VE/(cm3‚mol-1) ∆η/(mPa‚s)
toluene + propan-1-ol
VE/(cm3‚mol-1) ∆η/(mPa‚s)
toluene + butan-1-ol
VE/(cm3‚mol-1) ∆η/(mPa‚s)
toluene + pentan-1-ol
VE/(cm3‚mol-1) ∆η/(mPa‚s)
toluene + 2-methylpropan-2-ol
VE/(cm3‚mol-1) ∆η/(mPa‚s)
temp/K
ao
a1
a2
a3
σ
303.15 308.15 303.15 308.15 303.15 308.15 303.15 308.15 303.15 308.15 313.15 303.15 308.15 313.15 303.15 308.15 313.15 303.15 308.15 313.15 303.15 308.15 313.15 303.15 308.15 313.15 303.15 308.15 313.15 303.15 308.15 313.15
-0.394 -0.368 0.037 0.025 -0.116 -0.087 -0.546 -0.502 0.054 0.068 0.093 -1.525 -1.331 -1.172 0.384 0.443 0.521 -2.227 -1.897 -1.640 0.427 0.493 0.561 -3.180 -2.688 -2.276 2.093 2.118 2.166 -4.784 -3.516 -2.490
0.100 0.058 -0.186 -0.153 0.607 0.621 -0.036 -0.062 0.549 0.537 0.501 0.692 0.619 0.537 0.184 0.181 0.175 0.922 0.756 0.559 0.077 0.094 0.177 1.158 0.908 0.671 -0.830 -0.773 -0.739 3.9127 2.765 1.850
0.026 0.071 0.012 -0.006 0.024 0.083 -0.044 -0.048 -0.012 0.035 0.059 -0.076 0.065 0.238 -0.232 -0.243 -0.218 -0.284 -0.195 -0.056 0.063 0.113 0.186 -0.132 -0.061 0.051 0.915 1.054 1.084 -4.421 -3.150 -2.073
-0.080 0.020 0.017 -0.040 -0.238 -0.286 0.141 0.195 -0.059 0.018 0.130 -0.366 -0.425 -0.502 0.163 0.199 0.289 -0.270 -0.241 -0.094 0.053 0.076 0.0299 -0.233 -0.158 -0.080 0.878 0.805 0.895 2.608 1.840 1.060
0.002 0.002 0.002 0.001 0.008 0.008 0.005 0.005 0.003 0.004 0.005 0.006 0.006 0.008 0.007 0.006 0.005 0.008 0.008 0.008 0.004 0.005 0.003 0.005 0.005 0.007 0.027 0.025 0.026 0.017 0.014 0.011
where η12 is the viscosity of the mixture and x1, x2 and η1, η2 are the mole fraction and the viscosity of pure components 1 and 2, respectively. The estimated uncertainties are (0.002 cm3‚mol-1 for VE and (0.005 mPa‚s for ∆η. The results of VE and ∆η are fitted to the Redlich and Kister equation:13
Y ) x1x2
∑a (x i
1
- x2)i
(4)
where Y refers to VE/(cm3‚mol-1) or ∆η/(mPa‚s) and x1 and x2 are the mole fractions of toluene and alkanol, respectively. The coefficients ai were obtained by fitting eq 4 to experimental results using a least-squares regression
562
Journal of Chemical and Engineering Data, Vol. 45, No. 4, 2000 Table 4. Excess Molar Volumes (VE) and Deviations in Viscosity (∆η) at Equimolar Concentrations at (303.15, 308.15, and 313.15) K system toluene + methanol toluene + ethanol toluene + propan-1-ol toluene + butan-1-ol toluene + propan-1-ol toluene + 2-methylpropan-2-ol
(VE)
Figure 1. Excess molar volumes at 303.15 K for (x1) toluene + (1 - x1) alkanols: (.) methanol; (y) ethanol; (Q) propan-1-ol; (x) butan-1-ol; (K) pentan-1-ol; (i) 2-methylpropan-2-ol.
Figure 2. ∆η values at 303.15 K for (x1) toluene + (1 - x1) alkanols: (.) methanol; (y) ethanol; (Q) propan-1-ol; (x) butan1-ol; (K) pentan-1-ol; (i) 2-methylpropan-2-ol.
method. In each case, the optimum number of coefficients is ascertained from an examination of the variation in the standard deviation (σ). The calculated values of ai along with the tabulated standard deviations (σ) are given in Table 3. The σ was calculated using
σ)[
∑(Y
exp
- Ycal)2/(n - m)]1/2
(5)
where n is the number of data points and m is the number of coefficients. The variations of VE and ∆η with mole fraction of toluene (x1) for the six systems studied at 303.15 K are presented in Figures 1 and 2, respectively. The VE values are negative for the mixtures of toluene with methanol. For the mixtures of ethanol, propan-1-ol, or butan-1-ol, VE values are negative at lower mole fractions of toluene and positive at
temp/K
VE/(cm3‚mol-1)
∆η/(mPa‚s)
303.15 308.15 303.15 308.15 303.15 308.15 313.15 303.15 308.15 313.15 303.15 308.15 313.15 303.15
-0.098 -0.092 -0.029 -0.022 0.014 0.017 0.023 0.096 0.112 0.130 0.107 0.123 0.140 0.523
0.009 0.006 -0.136 -0.125 -0.381 -0.333 -0.293 -0.557 -0.447 -0.410 -0.795 -0.672 -0.569 -1.196
308.15 313.15
0.529 0.541
-0.879 -0.623
higher mole fractions of toluene. The VE values are positive over the entire composition range of binary mixtures containing pentan-1-ol or 2-methylpropan-2-ol. For equimolar mixtures (x1 = x2), VE varies as per the following order: methanol < ethanol < propane-1-ol < butan-1-ol < pentan1-ol < 2-methylpropan-2-ol. Also at equimolar composition, the VE values for toluene + propan-1-ol, + butan-1-ol, or + pentan-1-ol (0.014, 0.096, and 0.107 cm3/mol, respectively) agree with the reported values (0.035, 0.096, and 0.090 cm3/mol) of Swami et al.6 It has been reported14 that the VE values of binary mixtures result from the chemical, physical, and structural characteristics of liquids. Physical effects contribute to positive VE; chemical and structural effects contribute to negative VE. In the present systems, the negative VE values are attributed to changes in free volume in the mixture of electron donor-acceptor type interactions between alkanols and toluene (toluene being a π-electron donor). The positive VE arises due to breaking of H-bonds in the self-associated alcohol and steric hindrance due to the bulky methyl group in 2-methylpropan-2-ol. The sigmoidal shape of VE observed in the toluene + ethanol, + propan-1-ol, and + butan-1-ol systems is attributed to varying interactions between relatively large negative and positive contributions; their magnitudes are sensitive to the length of the component molecules. The VE values in the present study are found to increase with temperature, but this is not displayed in Figure 1. Figure 2 shows that ∆η is negative in all systems except for toluene + methanol and becomes more negative with increasing length and branching of alkanols. The temperature dependence of VE and ∆η at equimolar composition of all the systems studied is included in Table 4. Acknowledgment The authors are grateful to the Principal, M.S.G. College, Malegaon, for providing laboratory facilities and thankful to the Editor and reviewers for their constructive comments. Literature Cited Marsh, K. N.; Kim, E. S. Excess Enthalpies and Excess Volumes for 2-Methyl-2-propanol + Water at 5 K Intervals from 303.15 to 323.15 K. J. Chem. Eng. Data 1988, 33 (3), 288-292. Aminabhavi, T. M.; Banerjee, K. Density, Viscosity, Refractive Index, and Speed of Sound in Binary Mixtures of 1-Chloronaphthalene with Benzene, Methylbenzene, 1,4-Dimethylbenzene, 1,3,5-Trimethylbenzene, and Methoxybenzene at (298.15, 303.15, and 308.15) K. J. Chem. Eng. Data 1999, 44, 547-552.
Journal of Chemical and Engineering Data, Vol. 45, No. 4, 2000 563 Francesconi, R.; Castellai, C.; Comelli, F. Excess Molar Enthalpies and Excess Molar Volumes of Propylene Carbonate + Seven Pentanol Isomers at 298.15 K. J. Chem. Eng. Data 1999, 44, 144-147. Mather, A. E.; Maham, Y.; Teng, T. T.; Hepler, L. G. Volumetric Properties of (Water + Diethanolamine) Systems. Can. J. Chem. 1995, 73, 1514-1519. Gmehling, J.; deHaan, A. B. Excess Enthalpies for Various Binary Mixtures with N-Methylacetamide or Acetic Anhydride. J. Chem. Eng. Data 1996, 41, 474-478. Swamy, G. N.; Dhamaraju, G.; Raman, G. K. Excess Volumes of Toluene Mixtures with Some Alcohols at 303.15 K. Can. J. Chem. 1980, 58, 229-230. Moumouzias, G.; Ritzoulis G. Viscosities and Densities for Propylene Carbonate + Toluene at 15, 20, 25, 30, and 35 °C. J. Chem. Eng. Data 1992, 37, 482-483. Riddick, J. A.; Bunger, W. B. Techniques of Chemistry, 4th ed.; WileyInterscience: New York, 1986. Nikam, P. S.; Sawant, A. B.; Khairnar, R. S.; Aher, J. S. Limiting Partial Molar Volumes of (NH4)2SO4, K2SO4 and Al2(SO4)3 in Dimethylsulphoxide + Water at Different Temperatures. J. Mol. Liq. 1999, 81, 253-260. Nikam, P. S.; Sawant, A. B. Limiting Ionic Partial Molar Volumes of R4N- and Br- in Aqueous Acetonitrile at 298.15 K. J. Chem. Eng. Data 1997, 42, 585-589. Marsh, K. N. Recommended Reference Materials for the Realization of Physicochemical Properties; Blackwell Scientific Publications: Oxford, U.K., 1987. Nikam, P. S.; Shirsat, L. N.; Hasan, M. Density and Viscosity Studies of Binary Mixtures of Acetonitrile with Methanol, Ethanol, Propan1-ol, Propan-2-ol, Butan-1-ol, 2-Methylpropan-1-ol, and 2-Methylpropan-2-ol at (298.15, 303.15, 308.15, and 313.15) K J. Chem. Eng. Data 1998, 43, 732-737.
Redlich, O.; Kister, A. T. Algebric Representation of Thermodynamic Properties and the Classification of Solutions. Ind. Eng. Chem. 1948, 40, 345-348. Treszczanowicz, A. J.; Kiyohara, O.; Benson, G. C. Excess Volumes For n-alkanes Binary Mixtures of Decan-1-ol + n-Pentan, + nHexane, + n-Octane, + n-Decane, and + n-Hexadecane. J. Chem. Thermodyn. 1981, 13, 253-260. TRC Data Bases for Chemistry and Engineering: TRC Thermodynamic Tables, Ver. 1996-IS, Jan. 1996; Thermodynamic Research Center, Texas A & M University: College Station, TX, 1996. Zielkiewicz, J. Excess Molar Volumes and Excess Gibbs Energies in N,N-Dimethyl Formamide + Water, or + Methanol, or + Ethanol at the Temperature 303.15 K. J. Chem. Eng. Data 1998, 43, 650652. Venkatesu, V. P.; Rao, M. V. P. Excess Volumes and Viscosities of Tetrachloroethylene with Branched Alcohols at 303.15 K. J. Chem. Eng. Data 1996, 41, 819-820. Nikam, P. S.; Mahale, T. R.; Hasan, M. Densities and Viscosities for Ethyl Acetate + Pentan-1-ol, + Hexan-1-ol, + 3,5,5-Trimethylhexan1-ol, + Heptan-1-ol, + Octan-1-ol, and + Decan-1-ol at (298.15, 303.15, and 308.15) K. J. Chem. Eng. Data 1998, 43, 436-440. Aminabhavi, T. M.; Aralaguppi, M. J.; Shivaputrappa, B.; Harogoppad, B.; Balundgi, R. H. Densities, Viscosities, Refractive Indices, and Speeds of Sound for Methyl Acetate + Aliphatic Alcohols (C1-C8). J. Chem. Eng. Data 1993, 38, 31-39.
Received for review December 8, 1999. Accepted March 13, 2000.
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